CHAPTER 4.pptx
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The document discusses Lewis dot structures and bonding models. It begins by introducing the Lewis dot symbol notation for elements in the periodic table. It then explains the octet rule where atoms gain, lose or share electrons to achieve a full outer shell of 8 electrons. The document discusses different types of stability based on electronic configurations. It explains ionic bonding which results from electrostatic attractions between ions formed when a metal donates electrons to a nonmetal. Covalent bonding is described as the sharing of electrons between two nonmetals. Dative covalent bonding, also called coordinate bonding, involves the donation of a lone pair of electrons from one atom to an atom with an incomplete octet. Bond length relationships and exceptions to the octet rule
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![Octet Rule:
Tendency of atoms, other than H and He, to form bonds (by losing or gaining or
sharing electron ) until it is surrounded by eight valence electrons
Losing or gaining electron (Transferring electron)
Na + F Na+ [ F- ]
Sharing electron
F + F F F](data:image/gif;base64,R0lGODlhAQABAIAAAAAAAP///yH5BAEAAAAALAAAAAABAAEAAAIBRAA7)
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1). Chemical bonds form when atoms gain, lose, or share electrons to achieve stable noble gas configurations. Ionic bonds occur through electron transfer between metals and nonmetals, while covalent bonds form through electron sharing.
2). Lewis dot structures use dots to represent valence electrons and illustrate octet formations. Exceptions include expanded and incomplete octets. Molecular geometry is determined by minimizing electron pair repulsion using the VSEPR model.
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1). Chemical bonds form when atoms gain, lose, or share electrons to achieve stable electron configurations like the noble gas configuration. Lewis dot structures use dots to represent valence electrons and show electron sharing between atoms.
2). Ionic bonds form when a metal transfers an electron to a nonmetal, creating oppositely charged ions that are attracted to each other. Covalent bonds form when atoms share one or more pairs of electrons to achieve stable octets.
3). The VSEPR theory predicts molecular geometry based on electron pair-pair repulsion, treating bond pairs and lone pairs as electron domains around a central atom that arrange to maximize distance between each other. Common molecular geometries include linear, trigonal planar,
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CHAPTER 4.pptx
- 1. Lewis Dot Symbol Group 1 2 13 14 15 16 17 18 alence e- 1 2 3 4 5 6 7 8 ewis Dot Symbol Na Mg Al Si P S Cl Ar
- 2. Octet Rule: Tendency of atoms, other than H and He, to form bonds (by losing or gaining or sharing electron ) until it is surrounded by eight valence electrons Losing or gaining electron (Transferring electron) Na + F Na+ [ F- ] Sharing electron F + F F F
- 3. Types of Stability pe of stability Outermost Shell Example Electronic configuration of Its Most Stable Ion Noble gas onfiguration ns2 np6 Al (Z=13) alf-filled d- orbital onfiguration ns2 np6 nd5 Fe (Z=26) seudo-noble configuration ns2 np6 nd10 Zn (Z=30)
- 4. Formation of Ionic Bond (Electrovalent bond) Elements Combination: Metal and non-metal with big difference in electronegativity Formation: Electrostatic forces between positive and negative ions
- 5. Example Use Lewis dot symbols to show the formation of NaF. Na + F Na+ [ F ] • Na atom transfer its valence electron to F and forms Na+ ion • F atom accept electron from Na and forms F− ion • The electrostatic forces between Na+ and F− forms ionic bond. -
- 6. Elements Combination: Non-metal and non-metal with small difference in electronegativity Formation: Electrostatic forces between the shared electron with the nucleus of both shared atom Formation of Covalent Bond
- 7. Example Use Lewis dot symbols to show the formation of Cl2. Cl + Cl Cl Cl • Each Cl atom shared one electron to achieve octet • The electrostatic forces between the shared electron with the nucleus of both shared atom form a covalent bonds.
- 8. Formation: One of the atom donates both electrons Example Describe the formation of dative bond by using the reaction between NH3 and HCl N H H H + H Cl N H H H H + • Dative covalent bond formed when N atom contribute both electrons to H+ ion Cl - Formation of Dative Covalent Bond (Coordinate bond)
- 9. Bond Length single bond > double bond > triple bond C O > C O > C O
- 10. Lewis Structure 1: • Count the total no. of valence e- • Add e- (–ve) charge, subtract e- (+ve) charge 2: 3: 4: 5: • Draw skeletal structure of the compound • Put the least electronegative atom (except H & He) in the center • Count the number of e- which is used to form the covalent bonds and subtract from the total number of electrons. • Complete an octet (8 e- ) for all atoms except H & He (2 e- ) • If the central atom is not octet yet (except for B, Be, Al), make a multiple bond by using a lone pair from the surrounding atoms
- 11. Example Draw the Lewis structure for the following compound: (a) H2O (b) H3O+ (c) CO3 2-
- 12. Exception to Octet Rule complete Octet • Occurs when the central atom has less than 8e- in its valence shell. • Be, B and Al H Be H xpanded Octet • Occurs when central atom has more than 8e- in its valence shell. • Usually involves non-metal atoms of 3rd period and beyond - have empty 3d subshell. F S F d electron • Occurs when central atom contains an unpaired e- in its valence shell. N O F F F F